SubjectsSubjects(version: 941)
Course, academic year 2023/2024
Physical Chemistry B - B403002
Title: Fyzikální chemie B
Guaranteed by: Department of Physical Chemistry (403)
Faculty: Faculty of Chemical Engineering
Actual: from 2020
Semester: both
Points: 6
E-Credits: 6
Examination process:
Hours per week, examination: 3/2, C+Ex [HT]
Capacity: winter:unknown / unknown (unknown)
summer:unknown / unknown (unknown)Schedule is not published yet, this information might be misleading.
Min. number of students: unlimited
Language: Czech
Teaching methods: full-time
Teaching methods: full-time
For type: Bachelor's
Additional information:
Note: you can enroll for the course in winter and in summer semester
Guarantor: Kolafa Jiří prof. RNDr. CSc.
Class: Předměty pro fyzikální chemii
Interchangeability : N403040
This subject contains the following additional online materials
Annotation -
Last update: Kolafa Jiří prof. RNDr. CSc. (03.07.2020)
Course Physical Chemistry A+B provides a comprehensive overview of physical chemistry as a discipline used to understand the principles and calculations in chemistry and chemical engineering. The course begins with chemical thermodynamics and is based on a molecular point of view rather than on a classical continuous approach; therefore, the necessary basics of statistical thermodynamics are discussed in parallel. Part A (fall term) ends with phase equilibria. Part B (spring term) is devoted to chemical equilibrium, chemical kinetics, electrochemistry, and physical chemistry of surfaces. Other traditional fields of physical chemistry – quantum theory and spectroscopy – are not covered by the course.
Aim of the course -
Last update: Kolafa Jiří prof. RNDr. CSc. (03.07.2020)

Students will:

1. Understand fundamentals of chemical thermodynamics including basics of statistical thermodynamics,

2. Be able to apply methods of physical chemistry in a variety of fields of chemistry and chemical engineering;

3. Be able to formulate the problem, look for the necessary data in the literature, and communicate with experts more difficult tasks.

Literature -
Last update: Kubová Petra Ing. (04.12.2017)

R: Atkins P.W., de Paula J., Physical Chemistry, Oxford University Press, 2010, 9780199543373

Learning resources -
Last update: Kolafa Jiří prof. RNDr. CSc. (03.07.2020)

Syllabus -
Last update: Kolafa Jiří prof. RNDr. CSc. (03.07.2020)

15. Chemical equilibrium, reaction Gibbs energy, direction of reaction. Equilibrium constant and various methods of its calculation, dependence of equilibrium on temperature and pressure.

16. Methods of calculating equilibria (balance for one or more reactions, equation or a system of equations vs. minimization of Gibbs energy). Reactions in gas phase, with pure solid or liquid component, decomposition reactions. Solid phase reaction.

17. Reactions in electrolyte solutions, equilibria. Examples: strong and weak acids, hydrolysis of salts, buffers, pH calculations, speciation of ions, solubility of salts.

18. Formal chemical kinetics, reaction rate, kinetic equation, half-life, balance for simple and simultaneous reactions. Consecutive, parallel, and reversible reactions, relation to equilibrium (law of mass action). Kinetic measurements, determination of the order of reaction from rates and from the integrated form of the kinetic equation.

19. Potential energy surface, transition state, Arrhenius relation. Bonus: Eyring's equation and collision theory.

20. Reaction mechanisms and steady state approximation. Catalysis, enzymatic reactions (Michaelis and Menten mechanism), radical reactions. Bonus: Photon energy, photochemical reactions.

21. Electric bilayer, Poisson–Boltzmann equation, Gouy–Chapman model, Debye screening (solution of the linearized equation). Debye–Hückel theory of electrolyte solutions, applications.

22. Beketov series, electrolytic and galvanic cells, electrodes. Electrolysis and Faraday's law. Equilibrium galvanic cells, thermodynamics of reactions in a cell, Nernst equation.

23. Types of electrodes, galvanic cells as energy sources. Overpotential. Polarography, voltammetry. Corrosion and passivation.

24. Transport phenomena (in general), flow (masses, charges, etc.) and thermodynamic force. Diffusion: Fick's/Fourier's laws and heat conduction equations. Einstein–Smoluchowski and Einstein–Stokes equations, Brownian motion. Bonus: Entropy production, principle of minimal entropy production.

25. Ion migration in electrolyte solutions, conductivity, molar conductivity, ion mobility and relation to diffusivity. Kohlrausch's law. Conductivity measurement. Transference numbers. Bonus: Nernst layer, measurement of transference numbers.

26. Membranes. Osmotic pressure, van ’t Hoff equation, osmotic virial expansion (briefly). Electrical phenomena on membranes, Donnan equilibria. Non-equilibrium phenomena, Nernst-Planck equation, diffusion potential.

27. Interfaces. Interfacial energy and surface tension, curved interfaces, Laplace pressure, capillary action, Laplace–Young equation, Kelvin (Gibbs–Thomson, Ostwald–Freundlich) equation. Nucleation and spinodal decomposition (qualitatively). Surfactants, surface pressure. Micelles, films, colloids (briefly).

28. Adsorption. Physical adsorption and chemisorption. Common adsorption isotherms (Langmuir, BET, Freundlich). Capillary condensation. Bonus: Dissociative adsorption, Langmuir–Hinshelwood and Elye–Rideal mechanism.

Registration requirements -
Last update: Kubová Petra Ing. (04.12.2017)

Physical Chemistry A, Mathematics A, Mathematics B

Course completion requirements -
Last update: Kolafa Jiří prof. RNDr. CSc. (03.07.2020)

Credit C (calculations) at least 50%

Homework H at least 75%

Written test at least 40, oral max +20, total T min 50

Grade = 0.4×(C+H−50+T): F below 50, A for 90 or more; not better than D for test<50

Teaching methods
Activity Credits Hours
Konzultace s vyučujícími 0.5 14
Účast na přednáškách 1.5 42
Příprava na přednášky, semináře, laboratoře, exkurzi nebo praxi 1.5 42
Příprava na zkoušku a její absolvování 1.5 42
Účast na seminářích 1 28
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